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UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
General Certificate of Education Ordinary Level
* 2 0 6 6 5 3 7 1 1 2 *
5126/03
SCIENCE
Paper 3 Chemistry
October/November 2011
1 hour 15 minutes
Candidates answer on the Question Paper.
Additional Materials:
Answer Paper
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use a soft pencil for any diagrams, graphs, tables or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES.
Section A
Answer all questions.
Write your answers in the spaces provided on the question paper.
Section B
Answer any two questions.
Write your answers on the lined paper provided and, if necessary, continue on separate answer paper.
A copy of the Periodic Table is printed on page 12.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part question.
For Examiner’s Use
Section A
Section B
Total
This document consists of 9 printed pages and 3 lined pages.
DC (LEO/CGW) 38865
© UCLES 2011
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Section A
For
Examiner’s
Use
Answer all the questions.
Write your answers in the spaces provided on the question paper.
1
Complete Table 1.1 to list the uses of five materials and the reasons why each is chosen for
this use. One row has been completed for you as an example.
Table 1.1
material
use
reason for choice
silver salts
photography
turn black in sunlight
aluminium
calcium carbonate
diamond
helium
[8]
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2
Name the substances formed when the following changes take place.
For
Examiner’s
Use
(a) fermenting sugar
..................................................................
[1]
(b) melting zinc with copper
..................................................................
[1]
(c) reacting nitrogen and hydrogen
..................................................................
[1]
(d) adding chloride ions to silver nitrate solution
..................................................................
[1]
(e) removing an electron from a sodium atom
..................................................................
3
[1]
Name the pieces of apparatus best used to carry out the following procedures.
(a) Separate a precipitate from the solution in which it has formed.
..................................................................
[1]
(b) Determine the volume of a liquid.
..................................................................
[1]
(c) Change a vapour to a liquid.
..................................................................
[1]
(d) Add 17.3 cm3 of solution to a flask.
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[1]
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4
Fig. 4.1 describes the results of tests on four unlabelled metals, A, B, C and D.
Metal A
Metal B
Reacts explosively
with water.
Reacts with steam only
when very hot and with
dilute hydrochloric acid.
Metal C
Metal D
Reacts steadily with
cold water.
Does not react with
dilute hydrochloric acid.
For
Examiner’s
Use
Fig. 4.1
(a) Place the metals A, B, C and D in order of reactivity.
most reactive
..........
..........
..........
least reactive
..........
[2]
(b) Suggest a possible name for any three of the metals.
letter of metal
name of metal
(i)
(ii)
(iii)
[3]
© UCLES 2011
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5
Complete Table 5.1 with details of two homologous series.
For
Examiner’s
Use
Table 5.1
name of
homologous series
name of
example
structural
formula
characteristic
group of atoms
–OH
ethanol
H
carboxylic acids
H
C
H
C
O
H
O
[4]
6
(a) Write the name and chemical formula for
(i)
an acid,
name ................................................. chemical formula ..........................................
(ii)
an alkali.
name ................................................. chemical formula ..........................................
[2]
(b) Name the products of the reaction between the acid and alkali you have written in (a).
.............................................................. and ..............................................................[2]
(c) A substance forms ions when dissolved in water. Explain how the ions formed determine
whether the solution can act as an acid or an alkali.
..........................................................................................................................................
...................................................................................................................................... [3]
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7
An atom has an atomic number of 17 and a relative atomic mass of 35.
For
Examiner’s
Use
(a) Determine the number of protons and of neutrons in the nucleus of this atom.
protons ........................
neutrons ........................
[2]
(b) When atoms of this element form chemical bonds they form a stable electronic structure.
This can happen in two different ways. Describe each way.
1 .......................................................................................................................................
..........................................................................................................................................
2 .......................................................................................................................................
...................................................................................................................................... [4]
8
Vanadium, V, is extracted from a mineral called vanadinite. The chemical formula of vanadinite
is shown below.
Pb5(VO4)3Cl
(a) (i)
Calculate the relative molecular mass of vanadinite.
[Relative atomic masses: Ar: O, 16; Cl, 35.5; V, 51; Pb, 207]
relative molecular mass = ......................................................
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(ii)
Calculate the percentage by mass of vanadium in vanadinite.
For
Examiner’s
Use
percentage by mass = ......................................................
[3]
(b) In the extraction process, vanadinite is converted into vanadium(III) chloride, VCl 3.This
is reduced at a very high temperature by magnesium to form metallic vanadium and
magnesium chloride, MgCl 2.
(i)
Balance this equation for the reduction of vanadium(III) chloride by magnesium.
........ Mg + ........ VCl 3 → ........ V + ........ MgCl 2
(ii)
Calculate the mass of magnesium needed to produce 5 kg of vanadium.
[Relative atomic masses: Ar: Mg, 24; V, 51]
mass of magnesium = ................................................. kg
[3]
© UCLES 2011
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Section B
Answer any two questions.
Write your answers on the lined pages provided and, if necessary,
continue on separate answer paper.
9
(a) Fig. 9.1 describes reactions of a metal salt E.
blue solution
of metal salt
E
warm with
sodium hydroxide
solution and
aluminium
add
sodium hydroxide
solution
gas F
that turns damp
litmus paper
blue
dissolve
gas in
water
colourless
solution
G
blue
precipitate
H
Fig. 9.1
(i)
Identify E, F, G and H.
(ii)
Write an equation for any of the changes described in Fig. 9.1.
[6]
(b) Describe how pure crystals of E could be obtained from a dilute solution of E.
[4]
10 (a) Alkenes can be manufactured from alkanes obtained from petroleum. Briefly describe this
manufacturing process.
[4]
(b) Describe a laboratory test to distinguish between alkanes and alkenes.
[3]
(c) What volume of oxygen is needed to burn completely 10 dm3 of methane to carbon dioxide
and water? Show your working. All volumes are measured at room temperature and
pressure.
[3]
11 The Periodic Table on page 12 contains an element with proton number 3 and another element
with proton number 11.
(a) Identify these two elements and the group of the Periodic Table in which they are positioned.
[3]
(b) Give the electronic structures of these two elements. Use these to explain why both elements
appear in the same group of the Periodic Table.
[3]
(c) Another element, with the proton number 19, is in the same group of the Periodic Table as the
two elements in parts (a) and (b). For these three elements, suggest two similarities in their
properties and two trends in their properties.
[4]
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Examiner’s
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Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of
Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2011
5126/03/O/N/11
© UCLES 2011
Magnesium
Sodium
Calcium
5126/03/O/N/11
Strontium
Radium
45
89
89
Actinium
Ac
227
†
Hafnium
Key
b
X
a
b = atomic (proton) number
X = atomic symbol
a = relative atomic mass
72
Lanthanum
*
Hf
57
178
40
Zirconium
Zr
91
Titanium
139
Yttrium
Y
22
48
Ti
La
39
21
Scandium
Sc
* 58–71 Lanthanoid series
† 90–103 Actinoid series
88
Francium
87
226
Ra
223
Barium
Caesium
56
Ba
Cs
Fr
55
137
133
38
Rubidium
37
88
Sr
85
Rb
20
Potassium
19
40
Ca
39
12
24
Mg
23
Na
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
51
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
55
Tc
Re
186
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
27
59
28
59
29
64
30
65
5
Ru
101
Iron
Pm
147
Osmium
Os
190
237
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
Sm
150
Iridium
244
Pu
94
Plutonium
62
Eu
152
Platinum
243
Am
95
Americium
63
Europium
78
195
Pt
Ir
46
Palladium
Pd
106
Nickel
Ni
192
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
247
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
247
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
11
6
Dy
162
Thallium
Tl
204
Indium
251
Cf
98
Californium
66
Es
252
Holmium
Ho
165
Lead
Pb
207
Tin
99
Einsteinium
67
82
50
119
Sn
115
32
Germanium
Ge
73
Silicon
In
Gallium
Dysprosium
81
49
31
70
Ga
14
28
Si
Carbon
27
Aluminium
13
12
C
Al
Boron
B
7
14
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
257
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
8
Se
79
Sulfur
S
32
Oxygen
209
Po
169
Md
258
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
16
O
9
Yb
173
Astatine
At
210
Iodine
I
127
Bromine
Br
80
Chlorine
259
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
Lr
260
Lutetium
Lu
175
Radon
Rn
222
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
2
0
Hydrogen
VII
4
VI
He
V
1
IV
H
III
The volume of one mole of any gas is 24dm3 at room temperature and pressure (r.t.p.).
91
Protactinium
Thorium
231
Pa
Th
232
Praseodymium
Cerium
59
141
Pr
140
74
Tungsten
42
Molybdenum
24
Chromium
Cr
Ce
Tantalum
41
23
Vanadium
V
1
Group
DATA SHEET
The Periodic Table of the Elements
12